Q: A solution has a pH of 3. Which of the following statements is true?

The solution is acidic and has a high concentration of H\textsuperscript{+} ions.

Q: If a solution has a pH of 2, what is the concentration of hydrogen ions $$[\mathrm{H^+}]$$?

$$ 1 \times 10$$^{-2}$$ \ \mathrm{M} $$

Q: Which of the following best explains why pure water is neutral?

It contains equal concentrations of H\textsuperscript{+} and OH\textsuperscript{--} ions due to dissociation.

Q: If a solution has a pH of 9, what is its $$[\mathrm{H^+}]$$ concentration?

$$ 1 \times 10$$^{-9}$$ \ \mathrm{M} $$

Q: Which of the following would best describe the effect of adding a strong acid to a buffer solution?

The buffer would absorb excess H\textsuperscript{+} ions, minimizing the pH change.

Q: Which of the following is true about the pH scale?

It is a logarithmic scale measuring the concentration of H\textsuperscript{+} ions.

Question 1

Which of the following best describes a buffer in a biological system?

Accepted Answer

A solution that resists changes in pH by absorbing or releasing H	extsuperscript{+} ions.

Question 2

A solution has a pH of 3. Which of the following statements is true?

Accepted Answer

The solution is acidic and has a high concentration of H	extsuperscript{+} ions.

Question 3

Which of the following equations correctly represents the dissociation of water?

Accepted Answer

$$ \mathrm{H_2O} \rightarrow \mathrm{H^+} + \mathrm{OH^-} $$

Question 4

If a solution has a pH of 2, what is the concentration of hydrogen ions $$[\mathrm{H^+}]$$?

Accepted Answer

$$ 1 	imes 10$$^{-2}$$ \ \mathrm{M} $$

Question 5

Which of the following substances would have the highest pH?

Accepted Answer

Drain cleaner

Question 6

A solution with a pH of 6 has how many times lower H	extsuperscript{+} concentration than a solution with a pH of 2?

Accepted Answer

10,000 times

Question 7

Which of the following is a weak acid?

Accepted Answer

Acetic acid (CH\_3COOH)

Question 8

What is the pOH of a solution with $$[\mathrm{OH^-}] = 1 	imes 10$$^{-3}$$ \ \mathrm{M}$$?

Accepted Answer

$$ 3 $$

Question 9

A buffer system in blood involves carbonic acid and bicarbonate. Which equation best represents this system?

Accepted Answer

$$ \mathrm{CO_2$} + \mathrm{H_2O} \leftrightarrow \mathrm{H_2CO_3} \leftrightarrow \mathrm{H^+} + \mathrm{$$HCO_3$$^-} $$

Question 10

Which of the following best explains why pure water is neutral?

Accepted Answer

It contains equal concentrations of H	extsuperscript{+} and OH	extsuperscript{--} ions due to dissociation.

Question 11

A solution has $$[\mathrm{H^+}] = 1 	imes 10$$^{-8}$$ \ \mathrm{M}. $$What is its pH?

Accepted Answer

$$ 8 $$

Question 12

Which of the following is a strong base?

Accepted Answer

Sodium hydroxide (NaOH)

Question 13

If a solution has a pH of 9, what is its $$[\mathrm{H^+}]$$ concentration?

Accepted Answer

$$ 1 	imes 10$$^{-9}$$ \ \mathrm{M} $$

Question 14

Which of the following would best describe the effect of adding a strong acid to a buffer solution?

Accepted Answer

The buffer would absorb excess H	extsuperscript{+} ions, minimizing the pH change.

Question 15

Which of the following is true about the pH scale?

Accepted Answer

It is a logarithmic scale measuring the concentration of H	extsuperscript{+} ions.

Question 16

A solution with a pH of 11 is how many times more basic than a solution with a pH of 8?

Accepted Answer

1000 times

Question 17

Which of the following best describes the role of buffers in blood?

Accepted Answer

They maintain blood pH within a narrow range to support physiological functions.

Question 18

Which of the following is the correct formula to calculate pH from hydrogen ion concentration?

Accepted Answer

$$ \mathrm{pH} = -\log_{10}[\mathrm{H^+}] $$

Question 19

Which of the following would result in a solution becoming more acidic?

Accepted Answer

Increasing the concentration of H	extsuperscript{+} ions.

Acids, Bases, pH, and Buffering: Study Notes for General Biology

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